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Heat of Formation

What is the a...

Question

What is the amount of heat to be supplied to prepare $128 g$ of $C a C_{2}$ by using $C a C O_{3}$ and followed by reaction with carbon. Reactions are:
$C a C O_{3} (s) \to C a O (s) + C O_{2} (g); △ H^{o} = 42 .8 kcal$
$C a O (s) + 3 C (s) \to C a C_{2} (s) + C O (g); △ H^{o} = 111 kcal$

102.6 kcal

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221.78 kcal

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307.6 kcal

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453.46 kcal

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Solution

The correct option is C $307.6 kcal$
$C a C O_{3} (s) \to C a O (s) + C O_{2} (g) △ H^{0} = 42.8 kcal$
$C a O (s) + 3 C (s) \to C a C_{2} (s) + C O (g) △ H^{0} = 111 kcal$
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$C a C O_{3} (s) + 3 C (s) \to C a C_{2} (s) + C O (g) + C O_{2} (g) △ H = 153.8 kcal$

Thus heat required to prepare 1 mole of $C a C_{2}$ from $C a C O_{3}$
$= 153.8 kcal$
Molecular weight of $C a C_{2} = 40 + 24 = 64$
64 g of $C a C_{2}$ requires $153.8 kcal$ of heat
128 g of $C a C_{2}$ requires $307.6 kcal$ of heat

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Similar questions

C a C_{2}

C a C O_{3}

C a C O_{3} (s) \to C a O (s) + C O_{2} (g); △ H^{o} = 42 .8 k c a l

C a O (s) + 3 C (s) \to C a C_{2} + C O (g); △ H^{o} = 111 k c a l

How much heat will be required at constant pressure to form $1.28 k g$ of $C a C_{2}$ from $C a O (s)$ and $C (s)$ ?

Given:

$Δ_{r} H^{0} (C a O, s) = - 152 k c a l / m o l$ .

$Δ_{r} H^{0} (C a C_{2}, s) = - 14 k c a l / m o l$ .

$Δ_{r} H^{0} (C O, g) = - 26 k c a l / m o l$ .

2 k g

(C a C_{2})

C a O (s) + 3 C (s) \to C a C_{2} + C O (g)

C a O (s), C a C_{2} (s)

C O (g)

- 151.6, - 14.2, - 26.4 k c a l

I . C a C O_{3} (s) ⇌ C a O (s) + C O (g)

I I . M g (s) + 2 H_{2} O (g) ⇌ M g (O H)_{2} (a q) + H_{2} (g)

I I I . 2 N_{2} O_{5} (g) ⇌ O_{2} (g) + 4 N O_{2} (g)

How much heat will be required at constant pressure to form $1.28 k g$ of $C a C_{2}$ from $C a O (s)$ and $C (s)$ ?

Given:

$Δ_{r} H^{0} (C a O, s) = - 152 k c a l / m o l$ .

$Δ_{r} H^{0} (C a C_{2}, s) = - 14 k c a l / m o l$ .

$Δ_{r} H^{0} (C O, g) = - 26 k c a l / m o l$ .

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